In this work, the results of kinetic studies of the redox reaction of
gold(III) chloride complexes ([AuCl4]-) with formic acid, are presented.
Obtained data suggest the complex character of the reaction which leads to
the [AuCl2]- and [AuCl3(COOH)]- ions formation as intermediates. In the pH
range over 2.5, the final product of the reaction is metallic gold. From the
analysis of kinetic data, the rate limiting step is found to be the gold
metallic phase formation. The stage of Au(III) reduction is relatively fast
with the second-order rate constant equal to 61.8 M-1s-1 at temperature 50?C.
The rate of the studied reaction depends on the temperature, reactants
concentration and chloride ions concentration. As a result of the data
analysis, the scheme of the reaction path has been suggested. Also, the
values of enthalpy and entropy of activation for the reaction have been
determined.
Density of the copper-rich corner of the ternary Cu-Pb-Fe alloys was determined with the dilatometric method. Investigated alloys had constant copper content equal to 0.9, 0.8 and 0.7 mole fraction, and varied iron concentration up to 0.1 mole fraction. A model predicting the density of ternary solution from knowledge of density of pure component and the excess of molar volume for limiting binaries is proposed.
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